Test Bank for General Chemistry 10th Edition by Ebbing

Test Bank for General Chemistry 10th Edition by Ebbing Link full download: https://testbankservice.com/download/test-bank-for-general-che mistry-10th-edition-by-ebbing Chapter 9 - Ionic and Covalent Bonding 1. In which pair do both compounds exhibit predominantly ionic bonding? RbCl and CaO PCl 5 and HF KI and O 3 Na 2 SO 3 and BH 3 NaF and H 2 O ANS: A PTS: 1 DIF: easy REF: 9.1 OBJ: Define ionic bond. 2. The following representation of an atom is called a Lewis dot structure. an ion. a structural formula. an electrostatic potential map. an ionic bond. ANS: A PTS: 1 DIF: easy REF: 9.1 OBJ: Lewis electron-dot symbol. 3. Which of the following concerning Coulomb s law is/are correct? 1. The energy of an ionic bond is proportional to the size of the ion charges. 2. The energy of an ionic bond is inversely proportional to the distance between the charges. 3. The size of an ion is not important in determining the energy of an ionic bond. 1 only 2 only 3 only 1 and 2

1, 2, and 3 ANS: D PTS: 1 DIF: easy REF: 9.1 OBJ: Lewis electron-dot symbol. 4. When the cations Na +, K +, Rb +, Cs + are combined with chloride ion in the gas phase to form ion pairs, which pair formation releases the greatest amount of energy? KCl All release the same amount of energy. RbCl NaCl CsCl ANS: D PTS: 1 DIF: difficult REF: 9.1 OBJ: Describe the energetics of ionic bonding. KEY: properties of ionic substance 5. Which one of the following has an enthalpy change that is equal to the lattice energy of? ANS: E PTS: 1 DIF: easy REF: 9.1 OBJ: Define lattice energy. KEY: Born-Haber cycle 6. Which of the following statements concerning lattice energy is false? MgO has a larger lattice energy than NaF. The lattice energy for a solid with 2+ and 2 ions should be two times that for a solid with 1+ and 1 ions. MgO has a larger lattice energy than LiF. Lattice energy is often defined as the change in energy that occurs when an ionic solid is separated into isolated ions in the gas phase. All of these are true. ANS: B PTS: 1 DIF: moderate REF: 9.1 OBJ: Define lattice energy. KEY: Born-Haber cycle 7. Which of the following is a correct description of lattice energy? The energy change that occurs when electrons are removed from a lattice. The energy change that occurs when a gas condenses to a liquid. The energy change that occurs when a liquid freezes. The energy change that occurs when an ionic solid is separated into its ions in the gas phase.

The lattice energy of a substance is identical to the ionic bond energy determined from coulombs law. ANS: D PTS: 1 DIF: moderate REF: 9.1 OBJ: Define lattice energy. 8. In the Born Haber cycle for, which of the following processes corresponds to the first ionization energy of Na? ANS: D PTS: 1 DIF: easy REF: 9.1 OBJ: Describe the Born-Haber cycle to obtain a lattice energy from thermodynamic data. KEY: Born-Haber cycle 9. In the Born Haber cycle for, which of the following processes corresponds to the enthalpy of formation of? ANS: A PTS: 1 DIF: easy REF: 9.1 OBJ: Describe the Born-Haber cycle to obtain a lattice energy from thermodynamic data. KEY: Born-Haber cycle 10. In the Born Haber cycle for, which of the following processes corresponds to the electron affinity of F? ANS: E PTS: 1 DIF: easy REF: 9.1 OBJ: Describe the Born-Haber cycle to obtain a lattice energy from thermodynamic data. KEY: Born-Haber cycle

11. Which of the following processes is not exothermic? ANS: E PTS: 1 DIF: moderate REF: 9.1 OBJ: Describe the Born-Haber cycle to obtain a lattice energy from thermodynamic data. KEY: Born-Haber cycle 12. Calculate the lattice energy for LiF(s) given the following: sublimation energy for Li(s) DH f for F(g) first ionization energy of Li(g) electron affinity of F(g) enthalpy of formation of LiF(s) 1052 kj/mol 285 kj/mol 650. kj/mol 800. kj/mol none of these +166 kj/mol +77 kj/mol +520. kj/mol 328 kj/mol 617 kj/mol ANS: A PTS: 1 DIF: difficult REF: 9.1 OBJ: Describe the Born-Haber cycle to obtain a lattice energy from thermodynamic data. KEY: Born-Haber cycle 13. Which of the following compounds has the most ionic bonding (has the highest percentage of ionic character)? CaF 2 LiI OF 2 CsF LiF ANS: D PTS: 1 DIF: easy REF: 9.1 OBJ: Describe some general properties of ionic substances. KEY: properties of ionic substance 14. Which of the following compounds would be expected to have the lowest melting point? AlF 3 RbF NaF MgF 2

CaF 2 ANS: B PTS: 1 DIF: easy REF: 9.1 OBJ: Describe some general properties of ionic substances. KEY: properties of ionic substance 15. Which of the following compounds would be expected to have the highest melting point? CsF LiCl LiF NaBr CsI ANS: C PTS: 1 DIF: easy REF: 9.1 OBJ: Describe some general properties of ionic substances. KEY: properties of ionic substance 16. Which of the following compounds would be expected to have the highest melting point? NCl 3 OCl 2 MgCl 2 LiCl CCl 4 ANS: C PTS: 1 DIF: moderate REF: 9.1 OBJ: Describe some general properties of ionic substances. KEY: properties of ionic substance 17. Atoms of an element X have the ground-state electron configuration 1s 2 2s 2 2p 6 3s 2 3p 4. What type of ion is X most likely to form? X 6+ X 3 X 4+ X X 2 ANS: E PTS: 1 DIF: moderate REF: 9.2 OBJ: State the three categories of monatomic ions of the main-group elements. KEY: electron configurations of ions ions of the main-group elements 18. Which of the following is the Lewis dot structure for the rubidium ion?

ANS: E PTS: 1 DIF: easy REF: 9.2 OBJ: Write the electron configuration and Lewis symbol for a main-group ion. (Example 9.2) KEY: Lewis electron-dot symbol 19. Which of the following is the Lewis dot structure for the bromide ion? ANS: E PTS: 1 DIF: easy REF: 9.2 OBJ: Write the electron configuration and Lewis symbol for a main-group ion. (Example 9.2) KEY: Lewis electron-dot symbol 20. Which of the following is the Lewis dot structure for one formula unit of magnesium sulfide?

ANS: A PTS: 1 DIF: easy REF: 9.2 OBJ: Write the electron configuration and Lewis symbol for a main-group ion. (Example 9.2) KEY: Lewis electron-dot symbol 21. All of the following species have ground-state noble-gas electron configurations except Ge 4+ K + Kr I P 3 ANS: A PTS: 1 DIF: easy REF: 9.2 OBJ: Write the electron configuration and Lewis symbol for a main-group ion. (Example 9.2) KEY: electron configurations of ions ions of the main-group elements 22. Which of the following concerning the formation of ions is/are correct? 1. Elements with large electron affinities tend to form monoatomic anions. 2. No ionic compounds are found with positive ions having charges greater than the element group number. 3. Group 1A and 2A metals always have a positive charge equal to their group number in their ionic compounds. 1 only 2 only 3 only 1 and 2

1, 2, and 3 ANS: E PTS: 1 DIF: easy REF: 9.2 OBJ: Describe some general properties of ionic substances. 23. Which of the following concerning the formation of ions is/are correct? 1. Compounds of +4 ions are rare because of the large amount of energy required to form a +4 ion. 2. Some main group metals may have more than one possible positive charge because of the different energies required to remove s versus p valence electrons. 3. The nonmetals closest to the noble gases (Group 6A and 7 tend to form monatomic anions with noble gas configurations. 1 only 2 only 3 only 1 and 2 1, 2, and 3 ANS: E PTS: 1 DIF: easy REF: 9.2 OBJ: Describe some general properties of ionic substances. 24. All of the following have ground-state noble-gas electron configurations except Ar N 3 P 3+ Mg 2+ Cl ANS: C PTS: 1 DIF: easy REF: 9.2 OBJ: Write the electron configuration and Lewis symbol for a main-group ion. (Example 9.2) KEY: electron configurations of ions ions of the main-group elements 25. The formation of which monatomic ion of sulfur is the most energetically favorable? ANS: B PTS: 1 DIF: easy REF: 9.2 OBJ: Write the electron configuration and Lewis symbol for a main-group ion. (Example 9.2) KEY: electron configurations of ions ions of the main-group elements

26. What is the ground-state electron configuration of the ion? ANS: C PTS: 1 DIF: easy REF: 9.2 OBJ: Write the electron configuration and Lewis symbol for a main-group ion. (Example 9.2) KEY: electron configurations of ions ions of the main-group elements 27. What is the ground-state electron configuration of the sulfide ion? ANS: C PTS: 1 DIF: easy REF: 9.2 OBJ: Write the electron configuration and Lewis symbol for a main-group ion. (Example 9.2) KEY: electron configurations of ions ions of the main-group elements 28. What is the electron configuration for? ANS: A PTS: 1 DIF: easy REF: 9.2 OBJ: Write electron configurations of transition-metal ions. (Example 9.3) KEY: electron configurations of ions transition-metal ions 29. The Cr 2+ ion would be expected to have unpaired electrons. 4 2

3 0 1 ANS: A PTS: 1 DIF: easy REF: 9.2 OBJ: Write electron configurations of transition-metal ions. (Example 9.3) KEY: electron configurations of ions transition-metal ions 30. What is the electron configuration of? ANS: A PTS: 1 DIF: easy REF: 9.2 OBJ: Write electron configurations of transition-metal ions. (Example 9.3) KEY: electron configurations of ions transition-metal ions 31. What is the ground-state electron configuration of? ANS: C PTS: 1 DIF: easy REF: 9.2 OBJ: Write electron configurations of transition-metal ions. (Example 9.3) KEY: electron configurations of ions transition-metal ions 32. What is the ground-state electron configuration of? ANS: E PTS: 1 DIF: easy REF: 9.2 OBJ: Write electron configurations of transition-metal ions. (Example 9.3)

KEY: electron configurations of ions transition-metal ions 33. What is the ground-state electron configuration of the copper(i) ion,? ANS: D PTS: 1 DIF: easy REF: 9.2 OBJ: Write electron configurations of transition-metal ions. (Example 9.3) KEY: electron configurations of ions transition-metal ions 34. What is the ground-state electron configuration of? ANS: D PTS: 1 DIF: easy REF: 9.2 OBJ: Write electron configurations of transition-metal ions. (Example 9.3) KEY: electron configurations of ions transition-metal ions 35. All of the following ions have the ground-state electron configuration of a noble gas except which one? Ca 2+ Cl Ga 3+ Al 3+ H ANS: C PTS: 1 DIF: easy REF: 9.3 OBJ: Define isoelectronic ions. 36. Which set of ions are isoelectronic in their ground-state electron configurations? N, O, F, Ne Na +, K +, Rb +, Cs + F, Cl, Br, I Mg 2+, Ca 2+, Sr 2+, Ba 2+ N 3, O 2, Mg 2+, Al 3+ ANS: E PTS: 1 DIF: easy REF: 9.3

OBJ: Define isoelectronic ions. KEY: electron configurations of ions 37. Which of the following species is isoelectronic with Kr? Ar ANS: B PTS: 1 DIF: easy REF: 9.3 OBJ: Define isoelectronic ions. KEY: ionic radii 38. All of the following species are isoelectronic except Ar. Ca 2+. Mg 2+. Cl. S 2. ANS: C PTS: 1 DIF: easy REF: 9.3 OBJ: Define isoelectronic ions. KEY: ionic radii 39. Which pair of species is isoelectronic? Na + and K + K + and Cl Be 2+ and Na + Ne and Ar Li + and Ne ANS: B PTS: 1 DIF: easy REF: 9.3 OBJ: Define isoelectronic ions. KEY: ionic radii 40. Which two species are isoelectronic? Na + and K + Al 3+ and Ne P and Ca + Cl and F Ca 2+ and Mg 2+ ANS: B PTS: 1 DIF: easy REF: 9.3 OBJ: Define isoelectronic ions. 41. All of the following species are isoelectronic except S 2 K +

Na + Ar Cl ANS: C PTS: 1 DIF: easy REF: 9.3 OBJ: Define isoelectronic ions. 42. All of the following species are isoelectronic except O Ne N 3 Mg 2+ F ANS: A PTS: 1 DIF: easy REF: 9.3 OBJ: Define isoelectronic ions. 43. The following species,,, and, all have the same number of electrons. nucleons. neutrons. protons. isotopes. ANS: A PTS: 1 DIF: moderate REF: 9.3 OBJ: Define isoelectronic ions. KEY: ionic radii 44. Rank the following ions in order of decreasing atomic radii: Mo 4+, Mo 5+, Mo 6+. Mo 4+ > Mo 5+ > Mo 6+ Mo 6+ > Mo 5+ > Mo 4+ Mo 5+ > Mo 4+ > Mo 6+ Mo 6+ > Mo 4+ > Mo 5+ Mo 4+ > Mo 6+ > Mo 5+ ANS: A PTS: 1 DIF: easy REF: 9.3 OBJ: Use periodic trends to obtain relative ionic radii. (Example 9.4) 45. Rank the following ions in order of decreasing atomic radii: Te 2-, Te 4+, Te 6+. Te 2- > Te 4+ > Te 6+ Te 6+ > Te 4+ > Te 2- Te 4+ > Te 2- > Te 6+ Te 2- > Te 6+ > Te 4+ Te 4+ > Te 6+ > Te 2- ANS: A PTS: 1 DIF: easy REF: 9.3 OBJ: Use periodic trends to obtain relative ionic radii. (Example 9.4)

46. Which of the following species would you expect to have the largest radius? F ANS: D PTS: 1 DIF: easy REF: 9.3 OBJ: Use periodic trends to obtain relative ionic radii. (Example 9.4) KEY: ionic radii 47. In which of the following lists do the ions not appear in order of increasing ionic radius? S 2 < Cl < K + Na + < F < O 2 Cl < Br < I Li + < Na + < K + Al 3+ < Mg 2+ < Na + ANS: A PTS: 1 DIF: easy REF: 9.3 OBJ: Use periodic trends to obtain relative ionic radii. (Example 9.4) KEY: ionic radii 48. Rank the following ions in order of decreasing ionic radius: S 2, O 2, F, Na +, Mg 2+. S 2, O 2, F, Na +, Mg 2+ O 2, F, Na +, Mg 2+, S 2 O 2, S 2, F, Na +, Mg 2+ Mg 2+, Na +, F, O 2, S 2 Mg 2+, S 2, Na +, F, O 2 ANS: A PTS: 1 DIF: easy REF: 9.3 OBJ: Use periodic trends to obtain relative ionic radii. (Example 9.4) KEY: ionic radii 49. Rank the following species in order of decreasing radii: K +, Cl -, Se 2-, Br -. Br - > Se 2- > Cl - > K + Se 2- > Br - > Cl - > K + K + > Cl - > Se 2- > Br - Br - > Cl - > Se 2- > K + Cl - > Se 2- > K + > Br - ANS: B PTS: 1 DIF: easy REF: 9.3 OBJ: Use periodic trends to obtain relative ionic radii. (Example 9.4) 50. For which of the following pairs of species is the difference in radius the greatest? C and F K + and Br Li + and I

Na and Mg O 2 and F ANS: C PTS: 1 DIF: moderate REF: 9.3 OBJ: Use periodic trends to obtain relative ionic radii. (Example 9.4) KEY: ionic radii 51. Which of the following is the best explanation for a covalent bond? electrons simultaneously attracted by more than one nucleus an interaction between outer electrons the overlapping of unoccupied orbitals of two or more atoms the overlapping of two electron-filled orbitals having different energies a positive ion attracting negative ions ANS: A PTS: 1 DIF: moderate REF: 9.4 OBJ: Describe the formation of a covalent bond between two atoms. TOP: bonding covalent bonding 52. The formulas of many binary covalent compounds can be predicted on the basis that a bond is formed by the overlapping of two filled orbitals. that the number of bonds an atom can have is equal to the number of empty valence orbitals it has. that a bond is formed by the overlapping of atomic orbitals. that the number of bonds an atom can have is equal to the number of half-filled valence orbitals it can have. that bonding electrons are simultaneously attracted by more than one nucleus. ANS: D PTS: 1 DIF: moderate REF: 9.4 OBJ: Describe the formation of a covalent bond between two atoms. TOP: bonding covalent bonding 53. During the formation of a chemical bond between two hydrogen atoms, which of the following statements is always true? Energy is released during the formation of the bond. A polar covalent bond is formed. Electrons always are between the nuclei of the atoms. One of the hydrogen atoms is ionized. Resonance stabilizes the bond. ANS: A PTS: 1 DIF: moderate REF: 9.4 OBJ: Describe the formation of a covalent bond between two atoms. TOP: bonding covalent bonding 54. A bond in which both electrons of the bond are donated by one atom is called. a coordinate covalent bond a polar covalent bond an ionic bond a double bond a triple bond ANS: A PTS: 1 DIF: moderate REF: 9.4

OBJ: Define coordinate covalent bond. 55. A bond in which an electron pair is unequally shared by two atoms is polar covalent. coordinate covalent. ionic. nonpolar covalent. metallic. ANS: A PTS: 1 DIF: easy REF: 9.5 OBJ: Define polar covalent bond. TOP: bonding covalent bonding KEY: electronegativity polar covalent bond 56. The measure of the attraction that an atom has for the electrons in a chemical bond is called electronegativity. lattice energy. resonance energy. ionization energy. electron affinity. ANS: A PTS: 1 DIF: easy REF: 9.5 OBJ: Define electronegativity. TOP: bonding covalent bonding KEY: electronegativity 57. Which of the following atoms is the most electronegative? B N Al Cs Na ANS: B PTS: 1 DIF: easy REF: 9.5 OBJ: State the general periodic trends in the electronegativity. TOP: bonding covalent bonding KEY: electronegativity 58. An atom of which of the following elements has the highest electronegativity? K As Ba Si Br ANS: E PTS: 1 DIF: easy REF: 9.5 OBJ: State the general periodic trends in the electronegativity. TOP: bonding covalent bonding KEY: electronegativity 59. Which of the following concerning electronegativity is/are correct? 1. Differences in element electronegativities may be used to predict the type of

bonding, ionic or covalent, in a substance. 2. The larger the differences in electronegativity between two bonded atoms the more polar the bond. 3. The electrons in a polar bond tend to spend more time around the least electronegative element. 1 only 2 only 3 only 1 and 2 1, 2, and 3 ANS: D PTS: 1 DIF: moderate REF: 9.5 OBJ: Use electronegativity to obtain relative bond polarity. (Example 9.5) TOP: bonding covalent bonding 60. Which pair of elements would form a covalent bond that is the least polar? S and Li Al and N O and H O and F S and Cs ANS: D PTS: 1 DIF: easy REF: 9.5 OBJ: Use electronegativity to obtain relative bond polarity. (Example 9.5) TOP: bonding covalent bonding KEY: electronegativity polar covalent bond 61. Rank the following covalent bonds in order of decreasing polarity: C-H, N-H, O-H, F-H. F-H, O-H, N-H, C-H O-H, F-H, N-H, C-H N-H, F-H, O-H, C-H C-H, N-H, O-H, F-H C-H, F-H, O-H, N-H ANS: A PTS: 1 DIF: easy REF: 9.5 OBJ: Use electronegativity to obtain relative bond polarity. (Example 9.5) TOP: bonding covalent bonding 62. Which of the following bonds would be the least polar yet still be considered polar covalent? Mg-O C-O Si-O O-O N-O ANS: E PTS: 1 DIF: moderate REF: 9.5 OBJ: Use electronegativity to obtain relative bond polarity. (Example 9.5) TOP: bonding covalent bonding KEY: electronegativity polar covalent bond

63. In which of the following species is there the greatest unequal sharing of the bonding electrons? SO 3 SO 3 2 H 2 S H 2 O NH 4 + ANS: D PTS: 1 DIF: easy REF: 9.5 OBJ: Use electronegativity to obtain relative bond polarity. (Example 9.5) TOP: bonding covalent bonding KEY: electronegativity polar covalent bond 64. The Lewis formula for phosphine, PH 3, has four lone pairs. four bonding pairs. two bonding pairs and two lone pairs. three bonding pairs and one lone pair. one bonding pair and three lone pairs. ANS: D PTS: 1 DIF: easy REF: 9.6 OBJ: Write Lewis formulas with single bonds only. (Example 9.6) TOP: bonding covalent bonding KEY: Lewis dot formula 65. Which of the following concerning Lewis electron-dot formulae is/are correct? 1. A Lewis electron-dot formula (Lewis structure) is identical to a structural formula. 2. The skeleton of a molecule need not be known to draw the correct Lewis electron-dot structure. 3. Lewis electron-dot formulae show the location of bonding and nonbonding electrons in three dimensional space. 1 only 2 only 3 only 1, 2, and 3 none of the above ANS: E PTS: 1 DIF: easy REF: 9.6 OBJ: Lewis electron-dot structures. TOP: bonding covalent bonding 66. What is the total number of valence electrons in N 2 O 4? 34 11 16 17 46

ANS: A PTS: 1 DIF: easy REF: 9.6 OBJ: Write Lewis formulas with single bonds only. (Example 9.6) TOP: bonding covalent bonding 67. In the Lewis formula for difluorodiazine, N 2 F 2, the total number of lone electron pairs around the two nitrogen atoms is 4. 0. 3. 1. 2. ANS: E PTS: 1 DIF: easy REF: 9.6 OBJ: Write Lewis formulas having including multiple bonds. (Example 9.7) KEY: Lewis dot formula 68. Which of the following Lewis formulas is incorrect? ANS: B PTS: 1 DIF: easy REF: 9.6 OBJ: Write Lewis formulas having including multiple bonds. (Example 9.7) TOP: bonding covalent bonding KEY: Lewis dot formula 69. Which of the following is a correct Lewis electron-dot formula for H 2 SO 4?

ANS: A PTS: 1 DIF: easy REF: 9.6 OBJ: Write Lewis formulas having including multiple bonds. (Example 9.7) TOP: bonding covalent bonding 70. Which of the following is a correct Lewis electron-dot formula for CO? ANS: A PTS: 1 DIF: easy REF: 9.6 OBJ: Write Lewis formulas having including multiple bonds. (Example 9.7) TOP: bonding covalent bonding 71. Which one of the following has a Lewis formula most similar to that of NO? O 2 O 2 2 O 2 NO + NO ANS: A PTS: 1 DIF: moderate REF: 9.6 OBJ: Write Lewis formulas having including multiple bonds. (Example 9.7) TOP: bonding covalent bonding KEY: Lewis dot formula 72. The Lewis structure for each of the following except contains at least one double bond. O 2 CS 2 C 2 H 4

NO + N 2 H 2 ANS: D PTS: 1 DIF: easy REF: 9.6 OBJ: Write Lewis formulas having including multiple bonds. (Example 9.7) TOP: bonding covalent bonding KEY: multiple bonding 73. The Lewis structure for each of the following species except contains a triple bond. N 3 N 2 HCCH NO + O 2 2+ ANS: A PTS: 1 DIF: easy REF: 9.6 OBJ: Write Lewis formulas having including multiple bonds. (Example 9.7) TOP: bonding covalent bonding KEY: multiple bonds 74. How many valence electrons are present in the Lewis formula for the hypochlorite ion,? 20 12 18 14 16 ANS: D PTS: 1 DIF: easy REF: 9.6 OBJ: Write Lewis formulas for ionic species. (Example 9.8) TOP: bonding covalent bonding KEY: Lewis dot formula 75. What is the total number of valence electrons in the? 20 12 16 22 18 ANS: C PTS: 1 DIF: easy REF: 9.6 OBJ: Write Lewis formulas for ionic species. (Example 9.8) TOP: bonding covalent bonding KEY: Lewis dot formula 76. What is the total number of valence electrons in the nitrosyl ion,? 11 13 10

12 14 ANS: C PTS: 1 DIF: easy REF: 9.6 OBJ: Write Lewis formulas for ionic species. (Example 9.8) TOP: bonding covalent bonding KEY: Lewis dot formula 77. How many valence electrons are there in the tetraethylammonium ion,? 56 32 16 57 48 ANS: A PTS: 1 DIF: moderate REF: 9.6 OBJ: Write Lewis formulas for ionic species. (Example 9.8) TOP: bonding covalent bonding KEY: Lewis dot formula 78. What is the total number of valence electrons in the monohydrogen phosphate ion, 30 28 32 34 36? ANS: C PTS: 1 DIF: easy REF: 9.6 OBJ: Write Lewis formulas for ionic species. (Example 9.8) TOP: bonding covalent bonding KEY: Lewis dot formula 79. How many valence electrons does a nitrate ion have? 30 28 24 32 22 ANS: C PTS: 1 DIF: moderate REF: 9.6 OBJ: Write Lewis formulas for ionic species. (Example 9.8) TOP: bonding covalent bonding KEY: Lewis dot formula 80. How many valence electrons are there in the acetate ion,? 23 24 36

38 22 ANS: B PTS: 1 DIF: easy REF: 9.6 OBJ: Write Lewis formulas for ionic species. (Example 9.8) TOP: bonding covalent bonding KEY: Lewis dot formula 81. The total number of valence electrons in a peroxide ion,, is 2. 12. 14. 13. 15. ANS: C PTS: 1 DIF: moderate REF: 9.6 OBJ: Write Lewis formulas for ionic species. (Example 9.8) TOP: bonding covalent bonding KEY: Lewis dot formula 82. The number of valence electrons in the perfluoropropionate ion,, is 60. 62. 66. 80. 58. ANS: A PTS: 1 DIF: moderate REF: 9.6 OBJ: Write Lewis formulas for ionic species. (Example 9.8) TOP: bonding covalent bonding KEY: Lewis dot formula 83. The total number of valence electrons in the tetrathionate ion, S 4 O 6 2, is 58. 60. 56. 54. 62. ANS: E PTS: 1 DIF: moderate REF: 9.6 OBJ: Write Lewis formulas for ionic species. (Example 9.8) TOP: bonding covalent bonding KEY: Lewis dot formula 84. The number of valence electrons in the nitrite ion is 22. 16. 23. 18. 24.

ANS: D PTS: 1 DIF: easy REF: 9.6 OBJ: Write Lewis formulas for ionic species. (Example 9.8) TOP: bonding covalent bonding KEY: Lewis dot formula 85. The total number of valence electrons in the phosphate ion is 32. 30. 24. 28. 26. ANS: A PTS: 1 DIF: easy REF: 9.6 OBJ: Write Lewis formulas for ionic species. (Example 9.8) TOP: bonding covalent bonding KEY: Lewis dot formula 86. What is the total number of valence electrons in the sulfite ion? 30 26 24 8 32 ANS: B PTS: 1 DIF: moderate REF: 9.6 OBJ: Write Lewis formulas for ionic species. (Example 9.8) TOP: bonding covalent bonding KEY: Lewis dot formula 87. In the Lewis formula for hydrazinium ion, N 2 H 5 +, the total number of lone electron pairs around the two nitrogen atoms is 0. 4. 3. 1. 2. ANS: D PTS: 1 DIF: easy REF: 9.6 OBJ: Write Lewis formulas for ionic species. (Example 9.8) KEY: Lewis dot formula 88. In the Lewis formula for the hydroxide ion, OH -, the number of lone pairs of electrons around the oxygen atom is 3. 1. 2. 0. 4.

ANS: A PTS: 1 DIF: easy REF: 9.6 OBJ: Write Lewis formulas for ionic species. (Example 9.8) TOP: bonding covalent bonding 89. The concept of resonance describes molecular structures that have several different geometric arrangements. that have delocalized bonding. that are formed from hybridized orbitals. that have different molecular formulas. that have electrons resonating. ANS: B PTS: 1 DIF: easy REF: 9.7 OBJ: Define resonance description. TOP: bonding covalent bonding KEY: resonance 90. All the following statements about resonance are true except A single Lewis formula does not provide an adequate representation of the bonding. Resonance describes a more stable situation than does any one contributing resonance formula. Resonance describes the oscillation and vibration of electrons. The contributing resonance formulas differ only in the arrangement of the electrons. Resonance describes the bonding as intermediate between the contributing resonance formulas. ANS: C PTS: 1 DIF: easy REF: 9.7 OBJ: Define resonance description. TOP: bonding covalent bonding KEY: resonance 91. In which of the following species is resonance most likely to take place?

ANS: A PTS: 1 DIF: moderate REF: 9.7 OBJ: Write resonance formulas. (Example 9.9) TOP: bonding covalent bonding KEY: resonance 92. For the resonance hybrid of the nitrite ion, what is the average number of bonds between the nitrogen atom and an oxygen atom? 3/2 1 4/3 2 5/3 ANS: A PTS: 1 DIF: easy REF: 9.7 OBJ: Write resonance formulas. (Example 9.9) TOP: bonding covalent bonding KEY: resonance 93. Which one of the following species is best described by writing three equivalent Lewis formulas? SO 3 SF 4 SO 4 2 SO 3 2 SOF 4 ANS: A PTS: 1 DIF: difficult REF: 9.7 OBJ: Write resonance formulas. (Example 9.9) TOP: bonding covalent bonding KEY: resonance delocalization 94. For each of the following species except, the electronic structure may be adequately described by two resonance formulas. O 3 SO 3 2 NO 2 C 6 H 6 SO 2 ANS: B PTS: 1 DIF: easy REF: 9.7 OBJ: Write resonance formulas. (Example 9.9) TOP: bonding covalent bonding KEY: resonance delocalization 95. Which of the following are two appropriate resonance formulas for the acetate ion, CH 3 CO 2?

ANS: A PTS: 1 DIF: easy REF: 9.7 OBJ: Write resonance formulas. (Example 9.9) TOP: bonding covalent bonding KEY: resonance delocalization 96. The electronic structure of which of the following species cannot be adequately described by a single Lewis formula? CS 2 POF 3 HNNH NO 3 H 2 NNH 2

ANS: D PTS: 1 DIF: easy REF: 9.7 OBJ: Write resonance formulas. (Example 9.9) TOP: bonding covalent bonding KEY: resonance delocalization 97. Which of the following species represents an exception to the octet rule? SiO 2 HBr SF 4 PCl 3 CO 2 ANS: C PTS: 1 DIF: easy REF: 9.8 OBJ: Write Lewis formulas (exceptions to the octet rule). (Example 9.10) TOP: bonding covalent bonding KEY: exceptions to the octet rule 98. The Lewis structure of a molecule has a high probability of violating the octet rule if 1. the molecule has an odd number of valence electrons. 2. the central atom is surrounded by more than four atoms or eight valence electrons. 3. the central atom is from Group 2A or 3A. 1 only 2 only 3 only 1 and 2 1, 2, and 3 ANS: E PTS: 1 DIF: easy REF: 9.8 OBJ: Write Lewis formulas (exceptions to the octet rule). (Example 9.10) TOP: bonding covalent bonding 99. In which of the following molecules is the octet rule violated? SF 6 OF 2 ClF PF 3 SiF 4 ANS: A PTS: 1 DIF: easy REF: 9.8 OBJ: Write Lewis formulas (exceptions to the octet rule). (Example 9.10) TOP: bonding covalent bonding 100. The octet rule is violated by at least one atom in all the following compounds except SF 6. PF 6 -. BrF 5. ICl 2 -.

SiF 4. ANS: E PTS: 1 DIF: easy REF: 9.8 OBJ: Write Lewis formulas (exceptions to the octet rule). (Example 9.10) TOP: bonding covalent bonding 101. The Lewis formula of which species does not represent an exception to the octet rule? SiF 5 - SCl 6 SF 4 BF 3 CF 3 - ANS: E PTS: 1 DIF: easy REF: 9.8 OBJ: Write Lewis formulas (exceptions to the octet rule). (Example 9.10) TOP: bonding covalent bonding 102. Which species has the largest number of lone pairs of electrons around the central atom? XeF 2 XeF 6 XeOF 4 XeF 4 SiF 6 2 ANS: A PTS: 1 DIF: moderate REF: 9.8 OBJ: Write Lewis formulas (exceptions to the octet rule). (Example 9.10) TOP: bonding covalent bonding KEY: exceptions to the octet rule 103. In the Lewis formula for ClF 3, how many lone pairs are around the central atom? 0 4 3 2 1 ANS: D PTS: 1 DIF: easy REF: 9.8 OBJ: Write Lewis formulas (exceptions to the octet rule). (Example 9.10) TOP: bonding covalent bonding KEY: exceptions to the octet rule 104. Which of the following molecules has an incorrect Lewis formula?

ANS: A PTS: 1 DIF: moderate REF: 9.8 OBJ: Write Lewis formulas (exceptions to the octet rule). (Example 9.10) TOP: bonding covalent bonding KEY: exceptions to the octet rule 105. In the Lewis dot formula for ICl 2, the number of lone pairs of electrons around the central iodine atom is 2. 4. 1. 3. 0. ANS: D PTS: 1 DIF: moderate REF: 9.8 OBJ: Write Lewis formulas (exceptions to the octet rule). (Example 9.10) TOP: bonding covalent bonding KEY: exceptions to the octet rule 106. Which of the following has an incomplete octet in its Lewis structure? SO 2 F 2 NO 2 ICl CO 2 ANS: C PTS: 1 DIF: moderate REF: 9.8 OBJ: Write Lewis formulas (exceptions to the octet rule). (Example 9.10) TOP: bonding covalent bonding 107. Which of the following Lewis structures best describes BF 3?

ANS: C PTS: 1 DIF: easy REF: 9.8 OBJ: Note exceptions to the octet rule in Groups IIA and Group IIIA elements. TOP: bonding covalent bonding KEY: exceptions to the octet rule 108. Which of the following species represents an exception to the octet rule? BF 3 BF 4 CH 3 OH CCl 4 PH 3 ANS: A PTS: 1 DIF: easy REF: 9.8 OBJ: Note exceptions to the octet rule in Groups IIA and Group IIIA elements. TOP: bonding covalent bonding KEY: exceptions to the octet rule 109. From a consideration of the Lewis structure of the thiocyanate ion, SCN, in which carbon has a double bond with both the sulfur and nitrogen atoms, the formal charges on the sulfur, carbon, and nitrogen atoms are, respectively, 1, +1, 1. 2, 0, +1. 1, 0, 0. 2, +1, 0. 0, 0, 1. ANS: E PTS: 1 DIF: easy REF: 9.9 OBJ: State the rules for obtaining formal charge. TOP: bonding covalent bonding KEY: formal charge 110. Which of the following is/are true concerning formal charge? 1. The formal charge of each individual atom in a molecule or ion is an actual

atomic charge that can be experimentally determined. 2. The formal charge of each individual atom is always the same for each possible resonance form. 3. The sum of the formal charges of each atom in a molecule or ion equal the overall charge of the molecule or ion. 1 only 2 only 3 only 1 and 2 none ANS: C PTS: 1 DIF: easy REF: 9.9 OBJ: State the rules for obtaining formal charge. TOP: bonding covalent bonding 111. In the Lewis formula that minimizes formal charge, what is the formal charge on the sulfur atom in sulfur trioxide, SO 3? +2 +4 +6 2 0 ANS: A PTS: 1 DIF: easy REF: 9.9 OBJ: State the rules for obtaining formal charge. TOP: bonding covalent bonding KEY: formal charge 112. Which of the following statements is true concerning the Lewis formula that minimizes formal charge for H 2 SO 4? The formal charge of S is +2, the formal charge of each O is 0, and the formal charge H is 0. The formal charge of S is +2, the formal charge of O is either 0 or 2, and the formal charge of H is +1. The formal charge of S is +2, the formal charge of O is either 0 or 2, and the formal charge of H is 0. The formal charge of S is +2, the formal charge of O is 0, and the formal charge of H is +1. The formal charge of S is 0, the formal charge of O is 0, and the formal charge of H is 0. ANS: E PTS: 1 DIF: easy REF: 9.9 OBJ: State the rules for obtaining formal charge. TOP: bonding covalent bonding KEY: formal charge 113. In which of the following species is the octet rule violated by the central atom when the central atom has a formal charge of zero? SOCl 2

CCl 4 H 2 S PF 3 N 2 F 4 ANS: A PTS: 1 DIF: easy REF: 9.9 OBJ: State the rules for obtaining formal charge. TOP: bonding covalent bonding KEY: formal charge 114. What is the correct Lewis dot formula for sulfuric acid, H 2 SO 4, that minimizes formal charge? ANS: B PTS: 1 DIF: moderate REF: 9.9 OBJ: Use formal charges to determine the best Lewis formula. (Example 9.11) TOP: bonding covalent bonding KEY: formal charge 115. What is the formal charge on the chlorine atom in the chlorate ion, ClO 3, in the Lewis dot formula that minimizes formal charge? 2 +1 0

1 +2 ANS: C PTS: 1 DIF: moderate REF: 9.9 OBJ: Use formal charges to determine the best Lewis formula. (Example 9.11) TOP: bonding covalent bonding KEY: formal charge 116. In the Lewis dot formula that minimizes formal charge, how many bonds are there in the tetrathionate ion, S 4 O 6 2? 7 9 15 11 13 ANS: E PTS: 1 DIF: difficult REF: 9.9 OBJ: Use formal charges to determine the best Lewis formula. (Example 9.11) TOP: bonding covalent bonding KEY: formal charge 117. In the Lewis dot formula for the bromate ion (BrO 3 ) that minimizes formal charge, the central atom is surrounded by two bonding pairs and two lone pairs of electrons. four bonding pairs and one lone pair of electrons. three bonding pairs and no lone pairs of electrons. five bonding pairs and one lone pair of electrons. three bonding pairs and one lone pair of electrons. ANS: D PTS: 1 DIF: moderate REF: 9.9 OBJ: Use formal charges to determine the best Lewis formula. (Example 9.11) TOP: bonding covalent bonding KEY: formal charge 118. Which Lewis dot formula for pyrophosphate, P 2 O 7 4, minimizes formal charge?

ANS: A PTS: 1 DIF: moderate REF: 9.9 OBJ: Use formal charges to determine the best Lewis formula. (Example 9.11) TOP: bonding covalent bonding KEY: formal charge 119. As the number of bonds between two carbon atoms increases, which of the following decrease(s)? only the bond length only the bond energy only the number of electrons between the carbon atoms all of these none of these ANS: A PTS: 1 DIF: easy REF: 9.10 OBJ: Explain how bond order and bond length are related. (Example 9.12) TOP: bonding covalent bonding KEY: bond length 120. Which of the following statements is true? The triple bond in N 2 has a smaller bond order and a smaller bond length than the single bond in F 2. The triple bond in N 2 has a larger bond order and a smaller bond length than the single bond in F 2. The triple bond in N 2 has a smaller bond order and a larger bond length than the single bond in F 2. The triple bond in N 2 has a larger bond order and a larger bond length than the single bond in F 2. The triple bond in N 2 and the single bond in F 2 have the same bond order and the

same bond length. ANS: B PTS: 1 DIF: easy REF: 9.10 OBJ: Explain how bond order and bond length are related. (Example 9.12) TOP: bonding covalent bonding KEY: bond order 121. Which of the following species has the shortest bond distance? F 2 Cl 2 Br 2 I 2 H 2 ANS: E PTS: 1 DIF: moderate REF: 9.10 OBJ: Explain how bond order and bond length are related. (Example 9.12) TOP: bonding covalent bonding KEY: bond length 122. Which of the following diatomic species do you expect to have the longest bond length? O 2 + O 2 2 O 2 O 2 - they are all identical ANS: B PTS: 1 DIF: moderate REF: 9.10 OBJ: Explain how bond order and bond length are related. (Example 9.12) TOP: bonding covalent bonding KEY: bond length 123. Which of the following diatomic molecules has the greatest bond energy? H 2 HCl Cl 2 CO HF ANS: D PTS: 1 DIF: easy REF: 9.11 OBJ: Define bond energy. TOP: bonding covalent bonding KEY: bond energy 124. Consider the reaction 2HCl(g) H 2 (g) + Cl 2 (g); DH = 185 kj Which of the following statements is false? The reaction is endothermic. HCl(g) has a negative enthalpy of formation. The products have more enthalpy than the reactants. The HCl bond is longer than either the H 2 bond or the Cl 2 bond. The bond order of each of the products is one. ANS: D PTS: 1 DIF: easy REF: 9.11 OBJ: Define bond energy. TOP: bonding covalent bonding

KEY: bond energy 125. Using bond-energy data, what is DH for the following reaction? CH 4 (g) + 2Cl 2 (g) CCl 4 (g) + 2H 2 (g) Bond Bond Energy (kj/mol) C-H 413 H-H 432 Cl-Cl 242 C-Cl 328 40 kj 150 kj 40 kj 1415 kj 150 kj ANS: A PTS: 1 DIF: easy REF: 9.11 OBJ: Estimate delta H from bond energies. (Example 9.13) TOP: bonding covalent bonding KEY: bond energy 126. Using bond-energy data, what is DH for the following reaction? CH 3 OH(g) + H 2 S(g) CH 3 SH(g) + H 2 O(g) Bond Bond Energy (kj/mol) C-H 413 C-O 358 O-H 463 C-S 259 S-H 339 25 kj -124 kj 25 kj 2763 kj 2738 kj ANS: A PTS: 1 DIF: easy REF: 9.11 OBJ: Estimate delta H from bond energies. (Example 9.13) TOP: bonding covalent bonding KEY: bond energy 127. Based on the following data, what is the Br-Br bond energy? H 2 (g) + Br 2 (g) HBr(g); DH = 36.44 kj Bond Bond Energy (kj/mol) H-H 435 H-Br 362 399 kj/mol

216 kj/mol 216 kj/mol 289 kj/mol 289 kj/mol ANS: B PTS: 1 DIF: moderate REF: 9.11 OBJ: Estimate delta H from bond energies. (Example 9.13) TOP: bonding covalent bonding KEY: bond energy 128. Based on the following data, what is the bond energy of the C=C bond in 1,1-difluoroethylene, CF 2 CH 2? CH 4 (g) C(g) + 4H(g); DH = 1656 kj CF 4 (g) C(g) + 4F(g); DH = 1756 kj CF 2 CH 2 (g) 2C(g) + 2H(g) + 2F(g); DH = 2317 kj 611 kj/mol 845 kj/mol 820 kj/mol 1706 kj/mol 1910 kj/mol ANS: A PTS: 1 DIF: moderate REF: 9.11 OBJ: Estimate delta H from bond energies. (Example 9.13) TOP: bonding covalent bonding KEY: bond energy 129. Which of the following covalent molecules does not have the proper Lewis dot formula?

ANS: B PTS: 1 DIF: difficult REF: 9.9 OBJ: Use formal charges to determine the best Lewis formula. (Example 9.11) TOP: bonding covalent bonding KEY: Lewis dot formula 130. Use the bond energies provided to complete the following statement. when all of the bonds in acetic acid (CH 3 COOH) are broken. Bond Bond Energy (kj/mol) C-H 413 C-O 358 O-H 463 C=O 745 C-C 348 C=C 614 3153 kj/mol of energy is consumed 3153 kj/mol of energy is released 2805 kj/mol of energy is released 2805 kj/mol of energy is consumed 2766 kj/mol of energy is consumed ANS: A PTS: 1 DIF: easy REF: 9.11 OBJ: Estimate delta H from bond energies. (Example 9.13) TOP: bonding covalent bonding